4. CONCLUSION
By usinng solvothermal method, graphene nanoplatelets and its magnetic composite
MnFe2O4/GNPs were succesfully synthesized, as confirmed by XRD method. The condition of
reaction was studied and 200 °C was the proper temperature, at lower temperature, undesired
products were formed instead. The morphology and size of crystal were examined by SEM show
that MnFe2O4 has octahedral shape with size of about 30 nm, was in-situ deposited between
layers of GNPs sheets. Combining both material’s ability to remove lead ion from water, lead
absorption capacity of this composite was tested and the maximum absorption reached about
322.6 mg/g.
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Vietnam Journal of Science and Technology 56 (1A) (2018) 204-211
STUDY ON SYNTHESIS OF MnFe2O4/GNPs COMPOSITE
AND APPLICATION ON HEAVY METAL REMOVAL
Nguyen Duy Anh
Department of Inorganic Chemistry, Institute of Chemistry and Materials,
17 Hoang Sam, Cau Giay, Ha Noi, Viet Nam
Email: nguyen.duy.anh0@gmail.com
Received: 15 August 2017; Accepted for publication: 21 February 2018
ABSTRACT
Nowadays, composite materials between mixed-metal oxides and graphene are widely
studied due to their multiple applications on different fields. MnFe2O4 is a magnetic material
which has the ability to absorb toxic heavy metal in water. Graphene nanoplatelets (GNPs) with
about 10 layers, is one of type of graphene. GNPs was used as matrix for the fine distribution of
metal oxide nanoparticles. Surface area for the absorption process can be increased. Composite
was synthesized using solvothermal method, in which mixed-metal oxide nanoparticles were
directly formed in-situ from precursor salts onto GNPs surface. Synthesized material was
analyzed using XRD, SEM and EDX methods to determine its properties. Heavy metal
absorption capacity was also studied and showed good results.
Keywords: environmental treatment, MnFe2O4, GNPs, composite, solvothermal, heavy metal
absorption.
1. INTRODUCTION
In Vietnam, the rapidly growing industrialization and the fast growing factories lead to water
being contaminated toxic heavy metals. The exposure to these heavy metals is considered a major
health risk due to their toxicity and carcinogenicity. Among them, lead is a common
environmental pollutant. Lead exposure can occur from various routes like air, soil, commerical
products and especially from water. Causes of lead contamination often linked to industrial use of
lead, include factories and facilities that produce lead-acid batteries, lead wire and pipe, metal
recycling and foundries. Lead builds up in the body can damage brain and kidneys; in severe
cases anemia, coma and death may occur.
In recent years, nanoparticles of magnetic materials have been used to remove heavy metal
from water. These materials are useful because of their invaluable magnetic properties, such as in
magnetic seperation. Among them, MnFe2O4 have been proven to be a potential heavy metals
absorbent. Manganese ferrite have spinel structure and its properties depend on morphology and
size, which can be controlled by synthesis parameters [1]. Various methods are used to produce
Study on synthesis of MnFe2O4/GNPs composite and application on heavy metal removal
205
MnFe2O4 nanoparticles, such as solid state reactions [2], combustion synthesis [3], thermal
decomposition [4], coprecipitation [5] and hydrothermal method [6].
On the other hand, graphene nanoplatelets is multi-layered graphene, and thus it has many
interesting properties [7]. GNPs has many oxygenated function groups and high surface area,
which make it a good absorbent by nature. When combine together, MnFe2O4/GNPs composite
is a promising candidate for heavy metal removal, as material can be easily seperated out of the
water being treated using a magnet.
In this paper, the MnFe2O4/GNPs composite was synthesized by hydrothermal method, in
which the mixed-oxide particles were formed in-situ onto the GNPs surface. The purpose of this
method is to distribute evenly and avoid the agglomeration of oxide particles, thus increase the
surface area so the absorprion process is more effective.
2. EXPERIMENTAL
2.1. Preparation
2.1.1. Materials
Mn(NO3)2 50 % solution, Fe(NO3)3.9H2O 98.5 %, Pb(OAc)2.3H2O 99 %, K2S2O8 99.5 %,
H2SO4 98 %, EtOH 99.7 %, dimethylformamide DMF 99.5 % AR grade, graphite 99 % China
were used.
2.1.2. Preparation of GNPs
Graphite was first exfoliated partially by using method described in [8]. Typically, 2 g
graphite was dispersed in 100 mL solvent mixture containing 75 % acetone and 25 % H2O. The
mixture then was sonicated at 40 kHz and 300 W for 4 hours. The mixture was slightly heated for
solvent to evaporate to get the product.
Then, 2 g graphite from the first step was dispersed in 150 mL H2SO4 98 % and then 10 g
K2S2O8 was added. Thereafter, the reaction mixture was stirred for 4 hours at room temperature.
The GNPs product was then filtered out of the mixture, washed 3 times with ethanol, 3 times with
water, and finally dried at 60 °C for 6 hours.
2.1.3. MnFe2O4 and MnFe2O4/GNPs composite synthesis
Calculated amount of Mn(NO3)2 50 % solution and Fe(NO3)3.9H2O was measured and
dissolved in 60 mL dimethylformamide solvent so that concentration of Mn
2+
and Fe
3+
was
0.02 M and 0.04 M, respectively. The mixture was stirred for 30 minutes and then transfered to an
80 mL autoclave reactor, sealed and heated for 24 hours. Two different experiments were
conducted at 150 °C and 200 °C. Products were then filtered, washed 3 times with ethanol and
water, before being dried at 60 °C for 6 hours.
MnFe2O4/GNPs composite was formed by a similar process. First, 0.05 g GNPs was
dispersed in 60 mL DMF in 30 minutes at 40 kHz and 300 W. Second, Mn(NO3)2 and Fe(NO3)3
was added in the same amount as previous experiment. Last, the procedure was conducted at 200
°C for 24 hours.
2.1.4. Lead solutions
Nguyen Duy Anh
206
AR grade lead (II) acetate trihydrate was used to prepare stock solution of 400 mg/L. This
solution was diluted to get desired concentration at 200 mg/L, 100 mg/L, 40 mg/L, 20 mg/L, 10
mg/L.
2.2. Material characterization
The chemical composition of the material was characterized by Energy-dispersive X-ray
spectrometry (EDX) using Hitachi S-4800. The phase composition was determined by powder X-
ray diffraction (PXRD) method on X’Pert Pro. XRD patterns were recorded using CuKα radiation
(λ = 1.5406 Å). MnFe2O4 material has cubic crystal structure, space group 227: Fd-3m, lattice
parameter a = 8.5 Å [9]. The magnetic property of materials was checked simply by using a
magnet. The morphology of the material was characterized by scanning electron microscope
(SEM) using Hitachi S-4600. Lead concentration of after-treatment solution was measured by
atomic absorption spectroscopy (AAS) using contrAA 700.
2.3. Study on Pb
2+
absorption
Adding 0.01 g MnFe2O4/GNPs composite to 30 mL solution of each concentration prepared
above. The mixture was sonicated at 300 W and 40 kHz for 10 minutes, before being left for 20
hours to reach absorption equilibrium.
The amount of absorbed metal ion is calculated using the equation: qe = V.(C0-Ce)/m, where
qe (mg/g) is the amount of absorbed metal ions at equilibrium, C0 and Ce are initial concentration
and equilibrium concentration, respectively (mg/L), V (mL) is the volume of the Pb
2+
solution
and m (g) is the mass of the absorbent. The Langmuir isotherm between the amount of absorbed
metal ion and the concentration at equilibrium can be expressed by:
qe = bqmCe/(1+bCe)
where b is the Langmuir constant. This equation can be rewritten as:
Ce/qe = Ce/qm + 1/(bqm)
so qm can be calculated as 1/tanα from the plot between Ce/qe and Ce.
3. RESULTS AND DISCUSSION
3.1. Material characteristics
The material phase was identified by PXRD method (Figure 1a). Results showed that
synthesized GNPs still has characteristic peak of graphite, that is 26.7° corresponding to (002)
face (♦ symbol) of graphite but much lower intensity. The decrease of intensity indicate a loss of
crystalinity, as the result of the exfoliation of graphite. In addition, GNPs formation was also
indicated by great volume expansion and lower density.
Figure 1b shows XRD patterns of MnFe2O4. From lattice parameters [9], the peaks at
angles 2θ = 30°, 35.3°, 42.8°, 56.4° and 61.9°, correspond to (022), (113), (004), (115) and (044)
faces ( symbol), respectively. MnFe2O4 was synthesized without GNPs to optimize the
reaction conditions. At elevated temperature and with the presence of water, DMF was
hydrolyzed:
Study on synthesis of MnFe2O4/GNPs composite and application on heavy metal removal
207
HCON(CH3)2 + H2O → HCOOH + NH(CH3)2 (1)
also above boiling point, DMF decomposed as reaction:
HCON(CH3)2 → CO + NH(CH3)2 (2)
Dimethylamine was liberated, thus increase pH of the solution:
NH(CH3)2 + H2O → NH2(CH3)2
+
+ OH
-
(3)
At high pH, precursor salts were hydrolyzed to form hydroxides:
Fe
3+
+ 3 OH
-
→ Fe(OH)3
Mn
2+
+ 2 OH
-
→ Mn(OH)2
(4)
(5)
These hydroxides immediately lose water to form oxides at reaction temperature, at Fe
3+
: Mn
2+
ratio 2:1 manganese ferrite is formed:
Mn(OH)2 + 2 Fe(OH)3 → MnFe2O4 + 4 H2O (6)
This crucial process determined the outcome of the products. Both hydroxides have to be
formed simultaneously for reaction (6) to occur; otherwise, oxides of each metal were formed
seperately. Checking by using a magnet showed that only experiment with at 200 °C yields
magnetic products. Because Fe
3+
is much more easily hydrolyzed than Mn
2+
, if the pH rising was
not fast enough, hydrolyzation of Fe
3+
ions was preferred, so the main products were Fe2O3
(Figure 1c). This is the case when performing experiment at lower reaction temperature
(150 °C). At 200 °C, DMF decomposition rate was significantly faster, so both iron and
manganese nitrate salts hydrolyzed simutaneously with molar ratio 2:1 to form the desired
MnFe2O4 product. These conditions were chosen to perform next experiment with addition of
GNPs.
Figure 1. XRD patterns of a. MnFe2O4/GNPs composite, b. Fe2O3 formed at 150°C,
c. MnFe2O4 synthesized at 200 °C, d. GNPs.
Figure 1d shows XRD patterns of MnFe2O4/GNPs composite. Aside from peaks of
MnFe2O4, a peak at 26.7° was characteristic of GNPs indicating that the composite was
Nguyen Duy Anh
208
composed of both phases.
The morphology of synthesized GNPs and the composite material was characterized by
scanning electron microscope (SEM) (Figure 2).
Figure 2a,b show that the obtained GNPs has layer structure similar to that of graphite, but
with interlayer distance much wider, of about one micron and each layer thickness of about 20
nm. The large distance between each sheet contributed to the high surface area of material, and
is a neccesary condition for Fe
3+
and Mn
2+
to blend in while ultrasonicated mixture of GNPs and
salt precursors. Under hydrothermal condition, these salts deposited in-situ onto the surface of
GNPs layers, as seen in Figure 2c,d. In Figure 2c, it can be clearly seen that GNPs interlayer
distance and layer thickness was unchanged, so hydrothermal process did not effect GNPs itself,
but merely filled the gap between sheets with the mixed-oxides. The MnFe2O4 size and shape
can be seen in Figure 2d. The mixed-oxides crystal is uniform, narrow crystal size distribution of
about 30 nm. Compared to hydrothermal method in [6], the oxides particles were formed by in-
situ method had more well-defined shape. The reason is in this method, the crystal has more
time to growth, in which face (001) is preferred, result in slightly larger size but well-defined
octahedral shape.
(a) (b)
(c) (d)
Figure 2. SEM images of GNPs (a, b), MnFe2O4/GNPs compopsite side view (c),
MnFe2O4/GNPs composite top view (d).
Study on synthesis of MnFe2O4/GNPs composite and application on heavy metal removal
209
The chemical composition of the material was analyzed by Energy-Dispersive X-ray (EDX)
spectrometry and the results obtained are shown in Figure 3. It can be seen that the composition
varies on different areas. The mixed-oxides do not distribute evenly onto the GNPs surface.
However, elemental ratio between Fe and Mn in each area is roughly 2:1, which confirms the
formation of MnFe2O4. Note that the oxygen content is always larger than theoretical amount in
the oxides (4 times Mn content or 2 times Fe content). The exceeding amount (roughly 20 %) is
contributed to O in oxygenated GNPs and from water adsorbed into the material.
Figure 3. Energy-dispersive X-ray (EDX) spectroscopy of MnFe2O4/GNPs material.
3.2. Pb
2+
absorption
The maximum absorption capacity of the material was evaluated by using the Langmuir
absorption isotherm equation. In this study, the Pb
2+
concentrations were varied from 10 mg/L to
400 mg/L and a material amount was set to 0.01 g per 30 mL lead solution. After 20 hours
treatment, the absorption reached equilibrium. Then the material was seperated by using a
magnet, and lead concentration of the solutions was measured by AAS method. Results are
presented in Table 1.
Table 1. Pb
2+
absorption capacity of the MnFe2O4/GNPs material.
No. C0, mg/L Ce, mg/L qe, mg/g Ce/qe, g/L
1 10 0.4 28.8 0.014
2 20 1.5 55.5 0.027
3 40 4.2 107.4 0.039
4 100 20.2 239.4 0.084
5 200 111.0 267.0 0.416
6 400 295.0 315.0 0.937
Figure 4 was plotted from data in Table 1 between Ce and Ce/qe to estimate maximum lead
absorption capacity of the composite. The fitting line has R
2
value close to 1 so it is reliable. As
mentioned above, the maximum absorption value is the reciprocal of the fitting line’s tangent, and
Nguyen Duy Anh
210
can be calculated as qm = (0.0031)
-1
= 322.6 mg/g. This result is comparable with the results from
[6].
Figure 4. Graph of Langmuir isotherm equation.
As metal oxides containing oxygen atoms at outer surface of the crystals, Pb
2+
ions can be
attracted by electrostatic force with the negative charged oxygen. Lead also has affinity toward
metal oxides because of the hydroxide groups that remain on the surface. In this case, it is
especially true when the oxides were formed in hydrothermal environment. The remain of these
hydroxide groups can also be noticed, that XRD peaks of oxides prepared hydrothermally often
have low intensity, as the hydroxide decrease the crystallinity of the product. These hydroxide
groups can perform a substitute reaction with lead, in which hydrogen atoms are replaced with Pb
atoms, thus absorbing a good amount of lead in the process. GNPs provide a template for the
metal oxides to deposite on, evenly distribute those particles and by doing so increase the surface
exposure of the material. On the other hand, GNPs also has a minor contribution to the absorption
of lead atoms. By possessing various oxygenated groups: epoxy, hydroxide, carboxylate, which
have the same absorption mechanism as of the metal oxides, GNPs served the dual purposes as a
template and an absorbent.
4. CONCLUSION
By usinng solvothermal method, graphene nanoplatelets and its magnetic composite
MnFe2O4/GNPs were succesfully synthesized, as confirmed by XRD method. The condition of
reaction was studied and 200 °C was the proper temperature, at lower temperature, undesired
products were formed instead. The morphology and size of crystal were examined by SEM show
that MnFe2O4 has octahedral shape with size of about 30 nm, was in-situ deposited between
layers of GNPs sheets. Combining both material’s ability to remove lead ion from water, lead
absorption capacity of this composite was tested and the maximum absorption reached about
322.6 mg/g.
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